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3 years ago

What is true of a reaction that has reached equilibrium?

2 answers:

8 0

I believe the correct answer from the choices listed above is option A. A reaction that has reached equilibrium would mean that the reaction rates of the forward and reverse reactions are equal. Hope this answers the question. Have a nice day.

BabaBlast [244]3 years ago

4 0

The correct option is A.

A chemical reaction is said to have reached an equilibrium stage if the rate of reaction of the forward reaction is equal to the rate of reaction of the reverse reaction. Two way arrows are usually used to depict equilibrium reactions. These arrows indicate that the chemical reaction can move both ways. At the equilibrium point the concentrations of both the reactants and the products are equal.

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Your car burns gasoline as you drive from home to school

Vedmedyk [2.9K]

Yes,sr8 facts, mhm, agree

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3 years ago

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Why would the cell membrane shrink when the cells were placed in the 4% salt solution?

Elanso [62]

In a salt solution, the water potential is lower than that in the cell. In this case, water molecules will flow from a region of higher water potential to a region of lower water potential by osmosis. Which where water molecules is now flowing out of the cell to the salt solution. Because the cell lose so much water that it now shrinks.
Osmosis is where water molecules move down the water potential gradient through a semi permeable membrane, which is the cell membrane in this case.

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3 years ago

What element are diamonds composed of

never [62]

Answer:

diamonds are carbon based and have a giant covalent structure

Explanation:

This is what gives diamonds its strength and rigidity.

Diamonds are different from graphite due to the way the atoms are arranged

3 0

3 years ago

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1. How many moles of carbon are in 2.25 * 10^22 atoms of carbon ?

tresset_1 [31]

Answer:

atoms of C? 2.25 x 1022 atoms C x 1 mole C = 0.037 mol C

Explanation:

How many moles of C are in 2.25 x 1022 atoms of C?

3 0

3 years ago

Given the reaction has a percent yield of 86.8 how many grams of aluminum iodide would be required to yield an actual amount of

ioda

Answer:

Approximately $1.29 \times 10^3$ grams.

Explanation:

Let $x$ represent the number of grams of aluminum iodide required to yield that 73.75 grams of aluminum.

In most cases, the charge on each aluminum ion would be +3 while the charge on each iodide ion would be -1. For the charges to balance, there needs to be three iodide ions for every aluminum ion. Hence, the empirical formula for aluminum iodide would be $\rm AlI_3$ .

How many moles of formula units in that $x$ grams of $\rm AlI_3$ ? Start by calculating its formula mass $M(\mathrm{AlI_3})$ . Look up the relative atomic mass of aluminum and iodine on a modern periodic table:

Al: 26.982.
I: 126.904.

$M(\mathrm{AlI_3}) = 1\times 26.982 + 3\times 126.904 = 410.694\; \rm g \cdot mol^{-1}$ .

$n(\mathrm{AlI_3}) = \displaystyle \frac{m}{M} = \frac{x}{410.694}\;\rm mol$ .

Since there's one aluminum ion in every formula unit,

$n(\mathrm{Al}) = n(\mathrm{AlI_3}) = \displaystyle \frac{x}{410.694}\; \rm mol$ .

How many grams of aluminum would that be?

$m(\mathrm{Al}) = n \cdot M = \displaystyle \frac{x}{410.694}\; \times 26.982 = \frac{26.982}{410.694}\, x\; \rm g$ .

However, since according to the question, the percentage yield (of aluminum) is only $86.8\%$ . Hence, the actual yield of aluminum would be:

$\begin{aligned}&\text{Actual Yield} \\ &= \text{Percentage Yield} \times \text{Theoretical Yield} \\ &= 86.8\% \times \frac{26.982}{410.694}\, x \\ &= 0.868 \times \frac{26.982}{410.694}\, x \\ &\approx 0.0570263\, x\; \rm g\end{aligned}$ .

Given that the actual yield is 73.75 grams,

$0.0570263\, x = 73.75$ .

$\displaystyle x = \frac{73.75}{0.0570263} \approx 1.29 \times 10^3\; \rm g$ .

4 0

3 years ago